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Let           . Mark if the statement is true or false.           is an antiderivative of . [A]             is an antiderivative of . [B] Work does not have to be shown for this problem.

Let           . Mark if the statement is true or false.           is an antiderivative of . [A]             is an antiderivative of . [B] Work does not have to be shown for this problem.

Let           . Mark if the statement is true or false.           is an antiderivative of . [A]

Determine if each statement is true or false. The most general antiderivative of           is           .   [A] The most general antiderivative of            is           .  [B] Work does not have to be shown for this problem.

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.233 M. What is the value of Kc for this reaction?   CO(g) + Br2(g)  COBr2(g)  

For the reaction, 2SO2(g)  +  O2(g) 2SO3(g), at 900.0 K the equilibrium con­stant, Kc, has a value of 13.0.  Calculate the value of Kp at the same temperature.

When there is an increase in temperature of a system the rate of reaction often increases.  Which of the following best explains why this happens according to the collision theory?          1     The concentrations increase with temperature.        2     The number of collision with the sufficient kinetic energy increases with temperature.        3     The number of collisions per unit time increases with temperature.        4     The orientation of the molecules change with temperature.

Given the two reactions shown with their equilibrium constants,              PCl3(g)    +  Cl2(g)    –> PCl5(g)                                K1               2 NO(g)  +  Cl2(g)   –> 2 NOCl(g)                           K2         What is the equilibrium constant for the reaction,                    PCl5(g)  +  2 NO(g)  –> PCl3(g)  +  2 NOCl(g)

What is the molecularity of the following elementary reaction? NH2Cl(aq) + OH– (aq) → NHCl– (aq) + H2O(l)  

Nitrogen monoxide reacts with bromine at elevated temperatures according to the equation   2NO(g) + Br2(g)  –>  2NOBr(g)        In a certain reaction mixture the rate of formation of NOBr(g) was found to be 4.50 x 10‑4 mol L‑1 s‑1.  What is the rate of consumption of Br2(g)?